Explain why ethanol and acetone are not suitable solvents for extracting
organic compounds from aqueous solutions.
does it have to do with their density?
No, they are both 100% miscible with water, i.e. you get a single phase in all proportions.
The solvents ethanol and acetone are commonly used in laboratories due to their ability to dissolve a wide range of organic compounds. However, when it comes to extracting organic compounds from aqueous solutions, they may not be the ideal choices. The unsuitability of ethanol and acetone for this purpose is not primarily related to their density, but rather other important factors such as polarity and miscibility.
1. Polarity: Ethanol and acetone are polar solvents, meaning they have a significant degree of polarity. This polarity allows them to dissolve many organic compounds, which also tend to be polar or partially polar. However, in the case of aqueous solutions, water is a highly polar solvent, which could hinder the extraction process. When extracting organic compounds, it is generally preferred to use a nonpolar solvent to ensure efficient separation.
2. Miscibility: Another crucial factor to consider is the miscibility of the solvent with water. While both ethanol and acetone are miscible in water to some extent, the miscibility can cause challenges during the extraction process. Ideally, a solvent should form distinct layers with water to ease the separation of the organic compounds. Nonpolar solvents, such as dichloromethane or hexane, exhibit poor miscibility with water, allowing for a clear phase separation.
In summary, the unsuitability of ethanol and acetone for extracting organic compounds from aqueous solutions primarily results from their polarity and miscibility with water rather than their density. Nonpolar solvents are generally preferred to ensure efficient extraction and separation.